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Chemistry Review Sheet Unit 2 Phases of Matter 1. Match each arrangement of the particles in matter with a physical state. Physical State Arrangement ______ Gas a. packed tightly together ______ Liquid b. close, but free to flow ______ Solid c. spaced relatively far apart 2. What does the Kinetic molecular theory say about particle movement in each of the phases of matter? 3. Which of the substances are gases at 50oC? 4. Which of the substances are liquids at 50oC? 5. Which of the substances are solid at 50oC? 6. Which substance has the smallest temperature range as a liquid? 7. Types of Phase Changes (describe the phase change): a. Melting e. Vaporization b. Fusion f. Condensation c. Boiling g. Sublimation d. Evaporation h. Deposition 8. Identify the type of phase change for the following examples. a. H2O (l) H2O (s) d. H2O (l) H2O (g) b. H2O (s) H2O (l) e. H2O (g) H2O (l) c. H2O (s) H2O (g) f. H2O (g) H2O (s) Physical vs. Chemical Changes 9. Classify each of the following as a chemical or physical property. a. Reacts w/ water f. Dissolves in gasoline b. Is red g. Is ductile c. Conducts electricity h. Is flammable d. Resists corrosion i. Is 1.5 m long e. Boils at 88oC j. Freezes at -17oC 10. Classify each of the following as a chemical or physical change. a. Alcohol evaporating e. An explosion b. A firefly lighting up f. Salt dissolving in H2O c. A battery charging g. Digesting food d. Ice melting h. Hammering hot iron into a sheet Temperature Scales 11. Theoretically, all molecular motion ceases at what temperature? 12. How does the amount of energy required to change the temperature 1 oC compare to that of one Kelvin degree? 13. How can both a Celsius-scale thermometer and a Kelvin-Scale thermometer indicate the same temperature change but not the same final temperature reading? 14. Convert the following temperatures from one temperature scale to another as indicated. a. 516 K to oC d. 14K to oC o b. 155 C to K e. 421oC to K o c. 26 C to K f. 373 K to oC 15. Rank the following temperature readings in increasing order. 32oF, 32oC, 32 K, 102.1oC, 102.1j K Heat 16. What is the energy change associated with melting 9.14 kg of indium at 156.6oC? 17. How much energy is required to boil 4.66 kg of selenium at 685oC? 18. How much energy is required to condense 1.75 kg of sodium at 883oC? 19. State whether the following physical and chemical changes are endothermic or exothermic. a. Melting ________________ d. Fusion _________________ b. Vaporization ____________ e. Freezing _______________ c. Condensation ___________ f. Combustion ____________ 20. How many kilojoules of energy are in a donut that contains 200 Calories? 21. What is the specific heat of a substance that has a mass of 25 g and requires 525 calories to raise its temperature b y 15oC? 22. Suppose 100 g of H2O absorbs 1255.O J of heat. What is the corresponding temperature change? 23. How many joules of heat energy are required to raise the temperature of 100 g of aluminum by 120oC? The specific heat of aluminum is 0.90 J/goC. 24. Calculate the amount of heat needed to melt 35.0 g of ice at 0 oC. Express your answer in kilojoules. 25. Calculate the amount of heat needed to convert 190.0 g of liquid water at 18oC to steam at 100oC. 26. How much heat is absorbed when 28.3 g of water at 0oC is converted to liquid at 0 oC. 27. Determine the specific heat of a material if an 18 g sample absorbed 75 J as it was heated from 15 oC to 40oC. 28. How many grams of ice at 0oC can be melted into water at 0oC by the addition of 75.0 KJ of heat? ΔHfus for water = 6.01 kJ/mol 29. The amount of heat required to change the temperature of an object by exactly 1 oC is the object’s _______________________________. 30. Name each quantity that is represented in the equation for heat change in an aqueous solution. 32. What was the ΔT for the metal? 33. What was the ΔT for the water? 34. Calculate the heat change for the water. 35. Calculate the heat change for the metal. 36. Calculate the specific heat of the metal. 31. What was the final temperature of the metal? Separation techniques 37. How did you separate the mixture in lab? **hint ** what if iron was also mixed in there? Elements, Compounds and Mixtures 38. What is a diatomic molecule? Give an example. 39. Indicate which of the following is an element, compound, heterogeneous mixture or solution. a. Ocean water e. Copper i. Aluminum foil b. Calcium f. Grain alcohol j. Milk c. Vitamin C g. After-shave lotion k. Table salt d. Dry ice h. Hamburger l. Iron nail 40. 41. If represents Oxygen and represents hydrogen, illustrate what a water molecule would look like. 42. If represents salt, illustrate what an aqueous salt solution would look like. 43. Compare and contrast homogeneous and heterogeneous matter and give 2 examples. Heating curves 44. What is the physical state of substance A at room temperature? 45. What is the physical state of substance B at room temperature? 46. What is the melting point of substance A? 47. What is the melting point of substance B? 48. If you mixed substance A, substance B, and water and steadily increased the temperature, which would boil last?
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